1. Chapter 7: Reaction in Aqueous Solutions Reaction Types

2. Section 7.1 Predicting whether a Reaction will occur

3. 7.1 Predicting whether a reaction will occur What causes a reaction to “want” to occur? – Forming a solid – Forming water – Forming gas – Transferring electrons (Note: color change, energy released, etc. are SIGNS that a reaction has occurred, but do not say WHY a reaction would want to occur)

4. Section 7.2 Reactions that Form a Precipitate

5. Aqueous Solutions Aqueous Solutions: When compounds are dissolved in water they form aqueous solutions What does the word “dissolve” mean? – On a macroscopic level, when something dissolves, it looks like it disappears – What is happening on a molecular level depends on whether we’re talking about ionic or molecular compounds

6. Aqueous Solutions with MOLECULES MOLECULES (nonmetals only) do not break up into their elements when dissolved in water Example: sugar dissolves in water, but it DOES NOT break up into C, H, and O, it breaks up into individual C 6 H 12 O 6 molecules

7. Aqueous solutions with IONIC COMPOUNDS: IONIC compounds break up into the cation and the anion when they are dissolved in water The water contains the separated ions When it breaks up into its ions, the dissolved compound can conduct electricity An ionic compound that dissolves in water (not all ionic compounds do) it is called an electrolyte Example: NaCl in water

8. Example: Write the formula for barium nitrate: Is the compound ionic?? When barium nitrate dissolves in water, what will the solution look like? How many of each type of ion will barium nitrate produce? Write the formula for sodium carbonate. What will the solution look like after sodium carbonate dissolves? How many of each type of ion will be produced?

9. Sections 7.2 and 7.3 Double Replacement Reactions

10. Let’s say a chemist begins a reaction by dissolving Ba(NO 3 ) 2 and K 2 CrO 4 into water to form an aqueous solution… Are these compounds ionic? If so, what ions will the solution contain before the reaction? Draw a picture of the solution containing these ions below: If these two compounds react, what products do you think are likely to form from the reaction?

11. Think of the ions that are present in the solution. How could they get together to form new substances?

12. – The metals (cations) will be attracted to the nonmetals (anions) because opposite charges attract – Ba +2 and two NO 3 - ions could get together, but this would reform the reactants – If one Ba +2 and one CrO 4 -2 get together to form a compound, and one K+ and one NO 3 - get together to form a compound, then we will have NEW products – Write the ionic formulas for the products (CRIS-CROSS the charges): – Write and balance the equation between these two reactants. Be sure to account for the fact that this reaction takes place in water:

13. This reaction is called a double replacement reaction… Double Replacement Reaction: Occurs when atoms or ions from two different compounds replace each other. Format: AX + BY  AY + BX (A and B “switch partners”) *Do practice problems on double replacement reactions Predict the products for the following double replacement reactions: 1.sodium hydroxide + iron (III) chloride  2. Al 2 (SO 4 ) 3 + Mg(ClO 3 ) 2 

14. Section 7.3 Net Ionic Equations

15. Consider the balanced double replacement reaction that you wrote above between Ba(NO 3 ) 2 and K 2 CrO 4. Remember that many ionic compounds dissolve in water, and the compounds participating in the reaction can be written as ions. The equation you wrote is considered a molecular equation for the reaction Molecular Equation: shows the complete formulas of all the reactants or products Instead, we can write the ionic equation to get a more accurate picture of what is happening in the solution: Ionic Equation: the ions of the reactants and products are shown instead of the complete formulas

16. Write the ionic equation for the reaction between barium nitrate and potassium chromate: – Notice that in this equation, nothing really happens. The ions in the products look just like the ions in the reactants (maybe we wrote them in a different order, but nothing has changed).

17. When we get two compounds AX and BY together that dissolve in water, the ONLY ways to get a reaction are… 1. If a cation and an anion get together and they do NOT dissolve in water, then a precipitate is formed – Precipitate: solid that forms as a result from a reaction 2. If a cation and an anion get together and form water (like H+ and OH-) 3. If a cation and an anion get together and form a gas that exits the solution

18. When barium ions meet up with chromate ions in the solution, they form a solid. So, when a barium ion and a chromate ion find each other, a precipitate forms and the potassium ions and the nitrate ions are left behind in the solution

19. Consider the ionic equation that you wrote above for the reaction between barium nitrate and potassium chromate. Because the product barium chromate is a solid, it will not exist as separate ions at the end of the reaction. Write the ionic equation above to account for the new solid being formed:

20. Notice that in your equation, the potassium and nitrate exist as ions on both the reactant side and the product side of the reaction. These are spectator ions. Spectator ions: ions that do not participate in a reaction Just like in math class, when compounds exist on both sides of the equation, they can be “canceled out”. After canceling out the spectator ions, you can rewrite the net ionic equation for the reaction. Net Ionic Equation: includes only those components that are directly involved in the reaction.

21. Write the net ionic equation for the reaction between barium nitrate and potassium chromate:

22. NOTE: If both products for a reaction are aqueous, after the “  ” write N.R. for NO REACTION. If every ion is the same on both sides of the equation, no reaction occurred.

23. Write the balanced net ionic equation for the reaction between aqueous potassium hydroxide and aqueous iron (III) nitrate. NOTE: the compound containing iron after the reaction does not dissolve.

24. Write the balanced net ionic equation for the reaction between aqueous sodium chloride and aqueous lithium nitrate. Both products are aqueous.

25. Write the balanced net ionic equation for the reaction between aqueous ammonium chloride and aqueous lead (II) nitrate react to form a solid containing lead.

26. Section 7.2 Solubility

27. The term “solubility” refers to how easily something dissolves in water: Soluble solid: a solid that readily dissolves or dissociates into its ions in water Soluble solids are electrolytes in solution (form ions, can conduct) Insoluble solid (or slightly soluble solid): a tiny, tiny amount dissolves in water, but this amount is INVISIBLE to the naked eye Can you think of anything familiar that is insoluble in water?

28. In order to predict whether a precipitate will form from a double replacement reaction, we use the following solubility rules: Soluble (WILL dissolve)Exceptions (WON’T dissolve) Compounds w/ … Ionic compounds containing nitrate, chlorates, acetate Na +, K +, and NH 4 + salts Cl-, Br-, I- saltsCompounds w/ Ag+, Hg 2 2+, and Pb 2+ SO 4 2- Compounds w/ Ba 2+, Pb 2+, and Ca 2+ Insoluble (WON’T dissolve)Exceptions (WILL dissolve) Compounds w/ … S -2, CO 3 -2, PO 4 -3 saltsCompounds w/ H, Na, K, NH 4 + OH- saltsCompounds w/ group 1 metals, NH 4 + Ca +2, Ba +2  NOTE: in these rules, a “salt” refers to an ionic compound

29. Is it soluble?? Sodium hydroxide Aluminum chloride Silver nitrate Silver bromide Sodium carbonate Barium sulfate Barium hydroxide sodium carbonate **soluble potassium phosphate **soluble

30. Practice: For each of the following reactions… A. Predict the products for the reaction B. Write the balanced net ionic equation

31. Aqueous calcium nitrate and potassium hydroxide react.

32. Aqueous barium hydroxide reacts with sodium sulfate.

33. Aqueous iron (III) chloride reacts with lead nitrate.

34. Aqueous magnesium nitrate reacts with ammonium sulfate

35. Aqueous calcium chloride reacts with phosphoric acid

36. Section 7.4 Reactions that form Water

37. Acid: – Produces H+ in water – Seven acids are STRONG electrolytes (separate into ions). To be considered a strong acid, a compound needs to be a strong electrolyte. – Seven strong acids: MEMORIZE!! HCl HBr HI HNO 3 HClO 4 HClO 3 H 2 SO 4 – Weak acids do not completely dissociate (separate) into ions in solution

38. Base: – Produce an ion that accepts the H+ from an acid – Most common strong bases (strong electrolytes that separate completely into ions) produce the hydroxide ion when dissolved in water – Strong base examples: LiOH NaOH KOH Ba(OH) 2

39. Let’s look at a reaction between a strong acid and a strong base: Write the MOLECULAR equation for the reaction between aqueous nitric acid and sodium hydroxide: Now write the ionic equation for the reaction:

40. Based on the products of your reaction above, we see that a reaction between a strong acid and a strong base always produces liquid water and a salt. Salt = ionic compound Strong acid/base reactions are also considered to be double replacement reactions: – AX + BY  AY + BX – Where “A” is hydrogen, “Y” is hydroxide, and “AY” is water

41. Write the net ionic equation for the reaction between nitric acid and sodium hydroxide. NOTE: The hydrogen and hydroxide ion join together to form water… these ions will NOT be separated from each other in the solution. Because they’re not separated, we can’t cancel hydroxide and hydrogen ions out of our net ionic equation.

42. Practice – Write the balanced molecular equation for each of the following reactions between acids and bases. – Write the net ionic equation for each reaction.

43. Aqueous perchloric acid and potassium hydroxide react

44. Aqueous hydrochloric acid and barium hydroxide react

45. Aqueous sulfuric acid and sodium hydroxide react

46. Aqueous chloric acid and calcium hydroxide react

47. Section 7.5 Oxidation-Reduction Reactions

48. Red-ox reaction: Red-ox reaction: involves the transfer of electrons We will look at red-ox reactions with two different formats… FORMAT 1: – Write the balanced equation for the reaction between sodium metal and chlorine gas to produce solid sodium chloride:

49. What is happening when this reaction occurs?? Na metal is GIVING its 1 valence electron to one of the Cl atoms in chlorine gas – Na  Na+ + 1e- – Cl + 1e-  Cl- Na+ and Cl- form the ionic compound NaCl – Because electrons were GIVEN TO Cl, we say Cl was reduced (given negative charges) – Because electrons were TAKEN from Na, we say Na was oxidized

50. FORMAT 2: – Also called a single replacement reaction A + BX  AX + B Called single replacement b/c “A” replaces “B” in the compound – Write the balanced equation between solid aluminum and solid iron (III) oxide:

51. What’s happening when this reaction occurs?? Al metal has to LOSE 3 electrons to become part of the aluminum oxide ionic compound – Al  Al +3 + 3e- – Al has been oxidized Fe has to GAIN electrons to go from Fe +3 in the ionic compound to just plain Fe – Fe +3 + 3e-  Fe – Iron has been reduced

52. Some oxidation reduction reactions form a gas that bubbles out of solution Anytime a HONClBrIF is formed from a reaction, it will escape the solution as a gas – Example: Write the balanced equation for the reaction between hydrochloric acid and solid zinc:

53. Write the balanced equation for the reaction between solid sodium and hydroiodic acid.

54. NOTE: Some red-ox reactions involve electron transfer reactions between nonmetals (we won’t go over this in detail yet). For now know that the presence of oxygen as a reactant or product indicates that a red-ox reaction has occurred

55. Practice Problems a. Predict the products for the following oxidation-reduction reactions b. State which element was oxidized and which element was reduced for each example

56. Solid aluminum and iodine gas react Oxidized:Reduced:

57. Solid barium and cobalt (II) phosphate react Oxidized:Reduced:

58. Solid iron (III) and copper (II) chlorate react – Oxidized:Reduced:

59. Solid iron (III) and oxygen gas react Oxidized:Reduced:

60. Solid sodium and nickel (II) phosphate react Oxidized:Reduced:

61. Summary: Reactions we’ve Learned so Far

62. 1. Double replacement reactions: AX + BY  AY + BX A. Either have format… i.A solid precipitate is formed when two aqueous ionic compounds are mixed ii. A strong acid and a strong base produce water and a salt B. Need to be able to… i. Recognize the double replacement reaction and predict the products Recognize if the reaction produces a precipitate, liquid water, or if no reaction occurs Write the ionic and net ionic equation for the reaction

63. 2. Single replacement reactions and Red-Ox Reactions: a. Either have format… i. Metal + Nonmetal  Ionic Compound ii. A +BX  AX + B b. Need to be able to… i. Recognize a single replacement reaction or a red-ox reaction between a metal and a nonmetal ii. Predict the products for the reaction

64. Predict the products for the following reactions and write the balanced chemical equation. If no reaction occurs, write N.R. NOTE: If a polyatomic ion in the example is NOT included on your solubility rules, assume that compounds containing that ion ARE soluble

65. Practice Problems: DR and SR reactions 1. aqueous calcium acetate reacts with aqueous sodium carbonate 2. solid strontium reacts with iron (III) hydroxide 3. sodium nitrate reacts with phosphoric acid 4. sulfuric acid reacts with sodium hydroxide 5. aqueous barium hydroxide reacts with aqueous sodium phosphate 6. solid magnesium reacts with nitrogen gas 7. solid calcium reacts with solid copper (I) phosphate 8. aqueous calcium acetate reacts with aqueous potassium carbonate 9. solid copper (II) chloride reacts with solid potassium 10. aqueous calcium hydroxide reacts with aqueous calcium chlorate

66. Section 7.7 Other Reaction Types

67. A. Combustion Reactions Combustion reactions: involve oxygen and produce energy (heat). Usually occurs between a hydrocarbon and oxygen, and the products are ALWAYS simply carbon dioxide and water Combustion reactions follow the format below: C x H y + O 2  CO 2 + H 2 O C x H y O z + O 2  CO 2 + H 2 O – In both these examples, the compound containing C and H is the hydrocarbon – x, y, and z correspond to subscript numbers in the hydrocarbon

68. Write and balance the following equations: 1.When we light our Bunsen burners, a reaction occurs between methane (carbon tetrahydride) and oxygen in the air. Write the reaction for this process.

69. 2. When you barbeque, the propane (tricarbon octahydride) in your gas tank reacts with oxygen in the air.

70. B. Synthesis Synthesis (Combination) Reactions: a given compound is formed from simpler materials. In synthesis reactions, two or more reactants combine to form one product. Format: A + B  AB

71. Balance the following synthesis reactions 1. H 2 + O 2  H 2 O 2. N 2 + H 2  NH 3

72. C. Decomposition Reactions Decomposition Reactions: a single compound is broken down into simpler compounds or its component elements Format: AB  A + B Usually accomplished by heating a compound or passing an electric current through a compound Opposite of a synthesis reaction

73. Predict the products and balance the following decomposition reaction: MgF 2  NO 